a certain gas has a volume of 565 mL at 25 0C and 715 mm Hg.how many moles of gas are there?
To determine the number of moles of gas in this scenario, you will need to use the ideal gas law equation, which states:
PV = nRT
Where:
P = pressure of the gas (in atm)
V = volume of the gas (in liters)
n = number of moles of gas
R = gas constant (0.0821 L·atm/K·mol)
T = temperature of the gas (in Kelvin)
To solve for the number of moles of gas, we need to convert the given values to the appropriate units:
1. Convert the volume from milliliters (mL) to liters (L):
Given volume = 565 mL
1 L = 1000 mL
Volume in liters (V) = 565 mL / 1000 = 0.565 L
2. Convert the temperature from Celsius (°C) to Kelvin (K):
Given temperature = 25 °C
Temperature in Kelvin (T) = 25 + 273.15 = 298.15 K
3. Convert the pressure from millimeters of mercury (mm Hg) to atmospheres (atm):
Given pressure = 715 mm Hg
1 atm = 760 mm Hg
Pressure in atmospheres (P) = 715 mm Hg / 760 = 0.940 atm
Now, substitute the values into the ideal gas law equation:
PV = nRT
(0.940 atm)(0.565 L) = n(0.0821 L·atm/K·mol)(298.15 K)
Solving for n (number of moles of gas):
n = (0.940 atm)(0.565 L) / (0.0821 L·atm/K·mol)(298.15 K)
Calculate the right side of the equation:
n = 0.5042 mol (rounded to four decimal places)
Therefore, there are approximately 0.5042 moles of gas.